Final answer:
The compression factor (Z) is 1.12, indicating that the molar volume is 12% larger than predicted by the ideal gas law. To calculate the molar volume, use the ideal gas law with adjustments for the gas's non-ideal behavior, considering Z and the given conditions of temperature and pressure. Repulsive forces are dominating since Z is greater than 1.
Step-by-step explanation:
The question asks us to calculate two things for a gas that is not behaving ideally: (i) the compression factor (Z) under the given conditions, and (ii) the molar volume of the gas. Additionally, the question seeks an analysis of which forces, attractive or repulsive, are dominating in the sample.
To calculate the compression factor (i), we need to understand that Z is defined as the ratio of the actual molar volume (Vm) to the molar volume of the gas as predicted by the ideal gas law (Vm,ideal). The question states that the actual molar volume is 12 percent larger than the ideal calculation. Therefore, if Vm,ideal is taken as 100%, the actual volume Vm will be 112% of that value. Hence, Z will be 1.12.
(ii) To find the molar volume of the gas, we first calculate Vm,ideal using the ideal gas law (PV = nRT) where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. Assuming one mole of gas and rearranging the equation to solve for V (Vm,ideal = RT/P), we hold R as 0.0821 L*atm/mol*K, T as 350 K, and P as 12 atm. Thus, Vm,ideal is equal to (0.0821 L*atm/mol*K) * (350 K) / (12 atm) and the actual Vm is 12% larger than Vm,ideal.
The effects of intermolecular forces can be inferred from the compression factor value. A Z greater than 1 indicates that repulsive forces are dominating because the gas occupies a larger volume than predicted by the ideal gas law, which typically occurs at high pressures where the volume occupied by the molecules themselves becomes significant.